Ch 7 Section 2

Question 1

the charges on the ions composing an ionic compound reflect

Answer 1

the electron distribution of the compound

Question 2

in order to indicate the distribution of electrons among the bonded atoms in a molecular compound/polyatomic ion,

Answer 2

oxidation numbers (oxidation states), are assigned to the atoms composing the compound/ ion

Question 3

unlike ionic charges, oxidation numbers do not have an

Answer 3

exact physical meaning.

Question 4

oxidation numbers are useful in

Answer 4

naming compounds, writing formulas, and balancing chemical equations.

Question 5

as a general rule in assigning oxidation numbers, shared electrons are assumed to belong to

Answer 5

the more electronegative atom in each bond

Question 6

(Rules for determining oxidation numbers) the atoms in a pure element have an oxidation number of

Answer 6

zero

Question 7

(Rules for determining oxidation numbers) the more-electronegative element in a binary molecular compound is assigned the number equal to the

Answer 7

negative charge it would have as an anion

Question 8

(Rules for determining oxidation numbers) the less-electronegative atom is assigned the number equal to the

Answer 8

positive charge it would have as a cation

Question 9

(Rules for determining oxidation numbers) fluorine has an oxidation number of

Answer 9

-1 in all of its compounds because it’s the most electronegative element.

Question 10

(Rules for determining oxidation numbers) oxygen has an oxidation number of -2 in almost all compounds. Eceptions include when it is in

Answer 10

peroxides in which its ox # is -1, and when it’s in compounds with fluorine, in which its ox# is +2

Question 11

hydrogen has an ox number of +1 in all compounds containing elements that are

Answer 11

more electronegative than it; it has an ox # of -1 in compounds with metals

Question 12

(Rules for determining oxidation numbers) the algebraic sum of the oxidation numbers of all atoms in a neutral compound is

Answer 12

equal to zero

Question 13

(Rules for determining oxidation numbers) the algebraic sum of the oxidation numbers of all atoms in a polyatomic ion is equal to the

Answer 13

charge of the ion

Question 14

(Rules for determining oxidation numbers) rules apply to covalently bonded atoms but oxidation numbers can also be assigned to

Answer 14

atoms in ionic compounds

Question 15

(Rules for determining oxidation numbers) a monatomic ion has an oxidation number equal to the

Answer 15

charge of the ion

Question 16

because the sum of the oxidation numbers of atoms in a compound must be either zero / equal to charge of ion, it is often possible to

Answer 16

assign oxidation numbers when they are not known

Question 17

many nonmetals can have more than

Answer 17

one oxidation number

Question 18

these numbers can sometimes be used in the same manner as ionic

Answer 18

charges to determine formulas.

Question 19

a formula must represent

Answer 19

facts

Question 20

oxidation numbers alone cannot be used to prove the

Answer 20

existence of a compound

Question 21

the stock system is actually based on

Answer 21

oxidation numbers

Question 22

the stock system can be used as an alternative to the

Answer 22

prefix system for naming binary molecular compounds

Question 23

the stock system is more practical for

Answer 23

complicated compounds

Question 24

prefix-based names and stock-system names are still used interchangeably for

Answer 24

many simple compounds